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A&P 1 > Ch 2 Chemical Level of Organization > Flashcards

Ch 2 Chemical Level of Organization Flashcards

1
Q

Chemistry

A

the structure and interactions of all living matter

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2
Q

Matter

A

is anything that takes space and adds mass

3 states: solid, liquid, gas

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3
Q

Mass

A

is the amount of matter in an object

Mass does not change, weight does

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4
Q

Chemical elements

A

cannot be split into simpler substances

There are 118 elements, 92 occur naturally on Earth

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5
Q

Chemical symbols

A

consist of 1 or 2 letters of the elements name. Ex: Carbon=C, Oxygen=O, Hydrogen=H

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6
Q

Major Elements

A

make up 96% of body’s mass, they are oxygen(O), carbon, hydrogen(H), nitrogen(N)

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7
Q

Lesser elements

A

make up 3.6% body mass, calcium, phosphorus (P), potassium (K), sulfur (S), sodium chlorine (CI), magnesium (Mg), iron (Fe)

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8
Q

Atoms

A

smallest unit of matter, retain properties and characteristics of the element

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9
Q

Subatomic particles

A

compose individual atoms, they are protons, neutrons, and electrons

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10
Q

Protons

A

Positive charge

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11
Q

Neutron

A

no charge

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12
Q

Electron

A

negative charge

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13
Q

Electron shells

A

are circles around the nucleus that electrons orbit around.
Electrons fill into the shell in a specific order, innermost to outermost.
The number of electrons in an atom always equals the number of protons, each Atom is electrically neutral with a 0 charge

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14
Q

Atomic number

A

number of protons

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15
Q

Mass number

A

sum of protons and neutrons

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16
Q

Isotopes

A

are atoms with the same number of protons but different number of neutrons, this gives the atom a different mass number. Most isotopes are stable.

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17
Q

Radioactive Isotopes

A

are unstable and decay, releasing radiation.

They can transform into other elements when they decay. They can decay in 1 second or a million years

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18
Q

Half-life

A

half life of an isotope is the time it takes for half of the radioactive atoms in a sample to decay into a stable form

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19
Q

Dalton

A

(amu) is the unit used to measure atomic mass

Neutron has 1.008 dalton, proton has 1.007 dalton, electron has 0.0005 dalton

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20
Q

Atomic Mass

A

is the average mass of all naturally occurring isotopes

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21
Q

Ions

A

atoms that give up or gain an electron. Ex: Ca2+ stands for calcium with 2 positive charges b/c it lost 2 electrons

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22
Q

Ionization

A

the process of giving up or gaining an electron

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23
Q

Molecules

A

are when atoms share 2 electrons, chemically bonded

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24
Q

Compounds

A

contain atoms of 2 or more different elements. Ex: H2O and NaCI (sodium chloride

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25
Q

Free Radical

A

atom or group of atoms with an unpaired electron in outermost shell. These are unstable, highly reactive, and destructive. They become stable when they gain an electron or give the unpaired one away

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26
Q

Chemical Bonds

A

are forces that hold together atoms and molecules

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27
Q

Valence Shell

A

outermost shell, determines if atoms will form chemical bonds based on the number of electrons. If an atom is chemically stable it will not bond with another

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28
Q

Octet Rule

A

observation that elements tend to bond in such a way that each atom has eight electrons in its valence shell

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29
Q

Types of Chemical Bonds

A

ionic, covalent, hydrogen

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30
Q

Ionic Bonds

A

The force that holds together ions with opposite charges

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31
Q

Cation

A

positively charged ion, they lose an electron, ending up with more protons than electrons

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32
Q

Anion

A

negatively charged ion, they gain an electron, ending up with more electrons than protons

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33
Q

Covalent Bonds

A

Forms when 2 or more atoms share an electron. The larger the number of electrons shared, the stronger the bond

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34
Q

Single Covalent Bond

A

two atoms share one electron

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35
Q

Double Covalent Bond

A

two atoms share 2 pairs of electrons

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36
Q

Nonpolar Covalent Bond

A

two atoms share their electrons equally

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37
Q

Polar Covalent Bond

A

the electrons shared between two atoms is unequal

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38
Q

Electronegativity

A

the power to attract electrons to itself

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39
Q

Hydrogen Bonds

A

Forms when a hydrogen atom with a partial positive attracts the partial negative of near by atoms

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40
Q

Chemical Reaction

A

Occurs when new bonds form or old ones break

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41
Q

Reactants

A

the starting substance, Ex: H2 and O2

42
Q

Products

A

the end product, Ex: H2O

43
Q

Metabolism

A

all the chemical reactions occurring in the body.

44
Q

Potential Energy

A

energy stored by matter due to its position

45
Q

Kinetic Energy

A

energy associated with the matter in motion

46
Q

Chemical Energy

A

form of potential energy stored in bonds of compounds and molecules

47
Q

Law of Conservation of Energy

A

energy cannot be created or destroyed, but converted from one form to another

48
Q

Exergonic reactions

A

release more energy than they absorb

49
Q

Endergonic reactions

A

absorb more energy than they release.

50
Q

activation energy

A

The collision energy needed to break the chemical bonds of the reactants

51
Q

Concentration

A

The more particles of matter present in a confined space, the greater the chance that they will collide

52
Q

Temperature

A

As temperature rises, particles of matter move about more rapidly

53
Q

Catalysts

A

chemical compounds that speed up chemical reactions by lowering the activation energy needed for a reaction to occur

54
Q

Synthesis (anabolism)

A

2 or more atoms, ions, molecules combine to form larger molecules, synthesis means to put together
A+B = AB

55
Q

Decomposition (catabolism

A

splits larger molecules into smaller ones

AB= A+B

56
Q

Exchange

A

consists of synthesis and decomposition, switches partners

AB+CD= AD+BC

57
Q

Reversible

A

products can revert back to original reactants

AB = A+B and A+B = AB

58
Q

Oxidation-Reduction

A

breaks down food molecules to produce energy. Oxidation loses electrons and Reduction gains electrons. When one is oxidized the other is reduced at same time

59
Q

Inorganic Compounds

A

Lacks carbon, few atoms, cannot be used by cells for complicated functions, include water, salts, acids, and bases. Water is the most important inorganic compound.
Makes up 55-60% of body,
Inorganic compounds with carbon: carbon dioxide, bicarbonate, carbonic acid

60
Q

Organic Compounds

A

contain carbon, usually contain hydrogen, always has covalent bond. Large molecules made of long carbon atom chains
Makes up 38-43% of body

61
Q

Water

A

Most important compound in all living things. High polarity. Versatile solvent. Cohesive and can resist temp changes (high heat capacity)

62
Q

Solvent

A

does the dissolving. ex: water

63
Q

Solute

A

whats being dissolved. ex: salt

64
Q

Hydrophilic

A

water loving ex: salt or sugar

65
Q

hydrophobic

A

scared of water ex: oil/fats

66
Q

Dehydration synthesis

A

2 smaller molecules form larger, loss of water

67
Q

Mixture

A

compounds blended together but not bonded. Ex: air is made of nitrogen, oxygen, argon, carbon dioxide
3 types: solutions, colloids, suspensions

68
Q

Colloid

A

substance microscopically dispersed evenly throughout another substance. Appears translucent or opaque Ex: milk

69
Q

Suspension

A

can mix with liquid but will separate, ex: blood plasma

70
Q

Mass per volume

A

gives relative mass of solute found in volume of solution, Ex: “Alcohol 1% by volume”

71
Q

Moles

A

(mol/L) amount of substance that has mass in grams equal to sum of atomic mass in all atoms. Ex: 1 mole of chlorine (atomic mass= 35.45) is 35.45
Avogardros number is 6.023 x 10^23
Moles tell about # of atoms, ions or molecules present

72
Q

Dissociate

A

acids, bases, salts dissolve and separate into ions and surrounds by water molecules

73
Q

Acids

A

breaks off into hydrogen ions and anions, proton donor pH scale 1-6

74
Q

Bases

A

removes hydrogen, proton acceptor

75
Q

Salt

A

dissociates to cations and anions, electrolytes for carrying electrical currents

76
Q

pH scale

A

1-6 is acidic, 8-10 is a base, 7 is neutral

77
Q

Buffer System

A

convert strong acids/bases to weak ones

Maintenance of body fluid homeostasis is critical

78
Q

Carbon

A

organic compounds always contain carbon
Carbon can combine into many shapes
Carbon compounds do not dissolve easy in water
Carbon is good source of energy

79
Q

Macromolecules

A

small organic molecules combined into large ones

80
Q

Monomers

A

mono=one

the reaction that joins two monomers is a dehydration synthesis

81
Q

polymers

A

Poly=many, mers=parts
large molecule formed by the covalent bonding of many identical or similar small building‐block molecules called monomers

82
Q

Carbohydrate

A

“Watered carbon”
Includes sugars, glycogen, starches, and cellulose

Primary source of energy

Carbon, hydrogen, and oxygen are elements in carbs

3 groups: monosaccharides, disaccharides, polysaccharides

83
Q

monosaccharides

A

simple sugar, cannot be decomposed to simpler sugar, contain 3-7 carbon atoms

Glucose
Fructose(fruits)
Galactose (milk sugar)
Deoxyribose (DNA)
Ribose(RNA)
84
Q

disaccharide

A

2 or more monosaccharides

Sucrose (table sugar glucose+fructose), Lactose (milk sugar glucose+galactose)
Maltose (glucose+glucose)

85
Q

polysaccharides

A

tens to hundreds monosaccharides

Glycogen, Starch, Cellulose

86
Q

lipids

A

fats
hydrophobic
Types: fatty acids, triglycerides (fats and oils), phospholipids, steroids (ring of carbon atoms), eicosanoids (20 carbon lipids), fat soluble vitamins, lipoproteins

87
Q

Fatty Acids

A

synthesize phospholipids and triglycerides, can be saturated or unsaturated

88
Q

Saturated

A

contains one covalent bond, solid at room temp

89
Q

Unsaturated

A

one or more double covalent bonds, liquid at room temp

90
Q

Triglycerides

A

provide protection, insulation, energy
glycerol forms backbone of triglyceride
Solid or liquid at room temp

91
Q

Phospholipids

A

important in cell membranes
The “head: is hydrophilic
The “tail” is hydrophobic
Considered amphipathic (both polar and nonpolar)

92
Q

Steroids

A

includes all the sex hormones, adrenal cortical hormones, bile acids

93
Q

proteins

A

Give structure to body, regulate processes, provide protection, assist in muscle contraction, transport substances, serve as enzymes

Contain carbon, hydrogen, oxygen, nitrogen. Some contain sulfur

94
Q

amino acids

A

20 different amino acids, building blocks for protein
The covalent bond joining 2 amino acids makes a peptide bond
2 amino acids combine making a dipeptide, 3 make a tripeptide
10-2000 or more amino acids make polypeptide

95
Q

Enzymes

A

A catalyst in a living cell, highly specific, extremely efficient, subject to cellular controls, #1 Catalyst**
Protein part is called apoenzyme, non protein part is called cofactor

96
Q

Nucleic Acids

A

Make up DNA and RNA

Chain of repeating monomers called nucleotides

97
Q

DNA

A

forms genetic code in nuclei of cells and regulates most of the cells activities

98
Q

RNA

A

guides protein formation, relays instruction

99
Q

Nitrogenous base

A

4 different bases, adenine (A), thymine (T), cytosine [C], guanine (G)
A & T pair, C & G pair

100
Q

Pentose Sugar

A

five carbon sugar attached to base in DNA

101
Q

Phosphate group

A

form backbone of DNA

102
Q

Adenosine Triphosphate (ATP)

A

Principle energy storing molecule in the body
Usable energy is in 3rd phosphate
ATP is formed during cellular respiration
ATPases control the release of ATP

ATP moves ions across membrane during active transport
ATP is used in contraction of muscles

A&P 1 (1 decks)

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